The half-life of the first order reaction, A to products, is 53.2 s. What was the original concentration, (A)0 in moles per liter, if after 1.8 minutes, the concentration of A is 0.0783 moles per liter?

Not sure whether to use integrated rate law or half life law?

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  1. k = 0.693/t1/2
    Substitute into the expression below for k.
    ln(No/N) = kt.
    No = unknown
    N = 0.0783
    t = time. You must change this t to seconds if you use the half life in seconds or you can change the half life in seconds to minutes in which case you make use t in the lower equation in minutes.

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  2. Thank you!

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